Name: ___________________________________________________________________ Period: __________ CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW 1 Unit 1: Nature of Science Essential questions : What rules must be obeyed to safely conduct an experiment? What are the components of a good scientific experiment? What rules must be obeyed to safely conduct an experiment? Why are significant figures important to chemists? What is the best method/graph to represent specific data? How would a scientist organize data collected from an experiment into a graph? How does a standard notation number compare to a scientific notation number? How do you differentiate between accuracy and precision of data? Can you calculate % error of the results from an experiment? What are the SI base units? How is dimensional analysis used to convert units within the metric system? Why does the Big Bang Theory exist? Explain scientifically behind how the universe was created according to the Big Bang Theory? Key vocabulary : Scientific method Significant figures Metric system Base units Big Bang Theory Experiment Hypothesis Variable Control Accuracy Precision Percent error Practice : 1. Using the picture to the right, list lab safety rules that are being ignored. 2. What are the steps to the scientific method?
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Honors Chemistry Semester 1 Exam Review - www ...plantlectures.com/.../2011/08/ChemH.ExamReviewSem1.1112.pdfCHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW 1 Unit 1: Nature of Science Essential
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54. Which electrons are involved in bonding? _________________________________
55. What types of elements are involved in ionic bonding? ________________________ Covalent?___________________
56. What type of bond is formed by the transferring of electrons? ________________ Sharing electrons? ______________
57. How does an element form a cation?______________________________ Anion? _____________________________
58. Why does Magnesium form a +2 charge? _______________________________________________________________
59. How many valance electrons does each of the following elements have?
a) Sodium ________ b) Oxygen __________ c) Krypton __________
60. List the general characteristics of ionic and covalent bonds (i.e. physical properties (hardness, state of matter, boiling point, melting point, conductivity), strength)
Ionic
Covalent
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61. Using electronegativity values, what type of bond (ionic, polar covalent, nonpolar covalent) is formed between the following elements (show calculation):
b) F and F b) H and I c) Mg and Br d) C and Cl
62. How many electrons are shared in a: c) Single covalent bond ___ b) Double covalent bond ___ c) Triple covalent bond ___
63. Why do some elements form double and triple bonds during bonding? ________________________________________
64. Draw Lewis structures for the following. Identify the shape of the molecules (linear, bent, tetrahedral, trigonal planar and pyramidal). Identify the polarity of the molecules.
Molecule E-Dot Structure Shape Molecular
Polarity
Molecule E-Dot Structure Shape Molecular
Polarity
H2O
BF3
NFH2
PH3
CF4
CO2
Unit 6: Chemical Nomenclature
Essential questions:
How are ionic compounds identified?
What is a monatomic ion?
What are the common polyatomic ions’ names and formulas?
How are cations and anions combined to make ionic formulas?
How are Roman numerals used in ionic compound formulas?
How do you identify ionic compounds versus covalent (molecular) compounds?
What are the diatomic elements?
How are molecular formulas translated into binary covalent compound names? Key vocabulary:
Ionic compound Polyatomic ions Nonmetals
Covalent compound
Valence Electron
Ions
Cation
Anion
metals
Transition Metals
Octet rule
Binary Compound
Diatomic Molecules
Subscript
Superscript Practice: 65. Identify all seven diatomic elements: ___________________________________________________
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66. Write the formulas and charges for the following polyatomic ions: hydroxide: sulfate: phosphate: ammonium: nitrate: carbonate: 67. For the following ionic names, write the missing chemical formula or chemical name.
a. nickel (II) oxide _____________ b. calcium carbonate _____________
c. potassium nitrate _____________ d. ammonium bromide _____________
e. gold (III) iodide _____________ f. zinc phosphide _____________
g. lithium sulfate _____________ h. Na2SO4 ___________________________
i. Al2O3 ___________________________ j. SnO ___________________________
k. K2S ___________________________ l. (NH4)3PO4 ___________________________
m. ZnCl2 ___________________________ n. PbCO3 ___________________________
68. For the following molecular (covalent) compounds write the missing formula or name.
a. carbon monoxide ____________ b. xenon tetrafluroide ____________
c. silicon dioxide ____________ d. iodine pentachloride ____________
e. P2O5 ___________________________ f. P4O10 ___________________________
g. SF7 ___________________________ h. NI3 ___________________________
Unit 7: The Mole
Essential questions:
How is the mole used to count particles of a substance?
How does the mole relate to other everyday counting units?
Why is the mole used to count atoms instead of a more common unit?
How are moles of a substance converting to numbers of representative particles?
How is molar mass of a substance calculated?
How is the mass of an atom related to the mass of a mole of atoms?
How are moles of a substance converted to mass?
How are number of representative particles of a substance determined from its mass?
What is the difference between an empirical and molecular formula of a compound?
How is the percent composition of an element within a compound calculated?
How are empirical and molecular formulas obtained from percent composition data? Key vocabulary:
Mole
Atoms
Avogadro’s Number
Representative Particle
Hydrate
Molar Mass
Empirical Formula
Molecular Formula
Subscript
Percent composition
Practice:
Show all work for calculations:
69. Give conversion factors (in fraction form) for converting between the following
A.) FROM moles TO atoms B.) FROM grams TO moles of Boron C.) FROM atoms TO moles
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70. What is the molar mass of Rb2Cr2O7?
71. What is the % by mass of C in Pb(C2H3O2)2 ?
72. What is the molar mass of CoCl2 6H2O ?
73. What is the number of molecules in 16.75 g of H2O ?
74. What is the mass of 1.75 x 1024 molecules of NH3 ?
75. How many molecules are in 0.26 mol of CO2 ?
76. Which of the following are empirical formulas? H2O H2O2 C6H12O6 N2H5
Unit 8: Chemical Reactions
Essential questions:
What is evidence of a chemical change?
How is a chemical change different from a physical change?
How does a balanced chemical equation show relationships between the reactants and the product of a chemical reaction?
How can chemical reactions be classified?
What are the defining characteristics of each classification of chemical reaction?
What are aqueous reactions?
How are word equations translated into formula equations and vice versa? Key vocabulary:
Chemical Change
Physical Change
Coefficient
Molar Ratio
Conservation of Matter
Balanced Reaction
Chemical Reaction
Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
Aqueous Solution
Precipitate
Practice:
77. Differentiate between a precipitate and an aqueous solution. ______________________________________________